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A close relationship has been found between the standard entropies of elements and their electronic configurations. Based on the positions of elements in the periodic table and the variation in the standard entropies of elements, the standard entropies of elements can be expressed as the sum of two functions: S~0= f(N) + f(E), where S~0 is the standard entropy of an element, N the principal quantum number, and E the number of outermost electrons. And the specific formula is S~0=99.05N~1/3 + [0.32(sp - 4)~4 - 119.76] + [- 56.56N~1/3 + 0.70(sd - 7)~2 - 42.12]+[- 11.95 ×10~(-4)(df- 8)~4-105.70], where sp, sd, df are the numbers of the outermost electrons in the sp, sd, df regions of the periodic table, respectively. This formula helps reveal the essence of the standard entropies of elements and deepens our understanding of the thermodynamic characteristics of compounds.
Based on the positions of elements in the periodic table and the variation in the standard entropies of elements, the standard entropies of elements can be expressed as the sum of two functions: S~0 = f (N) + f (E), where S~0 is the standard entropy of an element, N the principal quantum number, and E the number of outermost electrons. And the specific formula is S~0 = 99.05N ~ 1/3 + [0.32 (sp - 4) ~ 4 ~ 119.76] + [-56.56N ~ 1/3 + 0.70 (sd ~ 7) ~2 ~42.212] + [- 11.95 × 10 ~ (- 4) (df-8) ~ 4-105.70] where sp, sd, df are the numbers of the outermost electrons in the sp, sd, df regions of the periodic table, respectively. This formula helps reveal the essence of the standard entropies of elements and deepens our understanding of the thermodynamic characteristics of compounds.